Lithium chloride is a chemical compound with a chemical formula “LiCl”. The salt is a normal ionic compound, although the Li+ ion is small in size, it produces unrecognized effects for other alkali metal chlorides, such as exceptional solubility in polar solvents and its hygroscopic properties.
IUPAC Name: Lithium chloride
Synonyms:
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Lithium chloride (LiCl)
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Lithium chloride
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LiCl
Molecular Formula: LiCl or ClLi
Molecular Weight: 42.4 g/mol
Properties:
1. Physical Properties of Lithium Chloride Licl:
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It is Deliquescent in nature, appear as cubic crystals, granules or crystalline powder
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It has sharp saline taste
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It has Boiling point of 2417 to 2480 °F at 760 mm Hg
Its Melting point is 1121 °F
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It has Density of 2.068 at 77 °F
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Aqueous solution of lithium chloride is neutral or slightly alkaline
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Solubility: Very soluble in water alcohols, ether, pyridine, nitrobenzene
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Solubility in Water |
68.29 g/100 mL (0 0C) |
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74.48 g/100 mL (10 0C) |
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84.25 g/100 mL (25 0C) |
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88.7 g/100 mL (40 0C) |
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123.44 g/100 mL (100 0C) |
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Solubility in Methanol |
45.2 g/100 g (0 0C) |
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43.8 g/100 g (20 0C) |
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42.36 g/100 g (25 0C) |
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44.6 g/100 g (60 °C) |
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Solubility in Ethanol |
14.42 g/100 g (0 0C) |
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24.28 g/100 g (20 0C) |
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25.1 g/100 g (30 0C) |
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23.46 g/100 g (60 0C) |
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Solubility in Formic Acid |
26.6 g/100 g (18 0C) |
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27.5 g/100 g (25 0C) |
2. Chemical Properties of Lithium Chloride Licl
When Lithium chloride reacts with sulfuric acid, it forms lithium sulfate and hydrogen chloride.
The chemical equation is given below.
[ 2LiCl + H_{2}SO_{4} rightarrow 2HCl + Li_{2}SO_{4}]
When lithium chloride reacts with sodium hydroxide, it forms lithium hydroxide and sodium chloride.
[ LiCl + NaOH rightarrow LiOH + NaCl]
Licl structure: lithium chloride structure
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Licl Lewis Structure:
lewis dot structure for Licl is shown below:
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Step-by-Step Explanation of How to Draw the Lithium Chloride Lewis Structure
Lithium chloride structure licl is drawn with the help of lewis dots
Lithium chloride is ionic compound, in which Lithium is a metal compound and chloride is a non-metal. Where electrons are transferred from metal ion to non-metal ion.
One electron is transferred from lithium and makes it electro-positive and by gaining one electron from lithium, chlorine becomes electronegative.
Preparation:
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Lithium chloride is prepared by treating lithium carbonate with hydrochloric acid. It is the highly exothermic reaction of lithium metal with either chlorine or anhydrous hydrogen chloride gas.
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When hydrate is heated along with a stream of hydrogen chloride, then anhydrous LiCl is produced
Uses of Lithium Chloride Licl:
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Lithium Metal by Electrolysis
Lithium chloride is primarily used at 450 ° C (842 ° F) for the preparation of lithium metal by electrolysis of a LiCl / KCl.
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As Brazing Flux
Lithium chloride is also used as a brazing flux for aluminum in automobile parts.
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Other Lithium Chloride Uses:
As desiccant in drying air streams.
lithium chloride is used in organic synthesis. For example, as an additive in the Stille reaction.
Biochemical Applications:
LiCl is used to precipitate RNA from cellular extracts
As a flame colorant, Lithium chloride is used to produce dark red flames.
Lithium chloride: it is used as a Relative humidity standard in the calibration of hygrometers and itself can be used as a hygrometer.
Molten LiCl is used for the preparation of lithium niobite, graphene and carbon nanotubes.
LiCl has strong acaricidal properties (Varroa destructor in populations of honey bees)